Answer:
approximately 48.26 grams of water are required to generate 35.0 grams of C₂H₂.
Explanation:
To determine the mass of water required to generate 35.0 g of C₂H₂, we need to use the balanced equation to establish the mole ratio between C₂H₂ and H₂O.
The balanced equation is:
CaC₂ + 2H₂O → C₂H₂ + Ca(OH)₂
From the equation, we can see that 1 mole of C₂H₂ is produced from 2 moles of H₂O.
To calculate the number of moles of C₂H₂, we divide the given mass of C₂H₂ (35.0 g) by its molar mass (26.04 g/mol):
Moles of C₂H₂ = 35.0 g / 26.04 g/mol ≈ 1.34 mol
Using the mole ratio from the balanced equation, we can determine the moles of H₂O required:
Moles of H₂O = 1.34 mol * (2 mol H₂O / 1 mol C₂H₂) ≈ 2.68 mol
Finally, we can calculate the mass of H₂O by multiplying the moles of H₂O by its molar mass (18.02 g/mol):
Mass of H₂O = 2.68 mol * 18.02 g/mol ≈ 48.26 g
Therefore, approximately 48.26 grams of water are required to generate 35.0 grams of C₂H₂.
